From the following heats of reaction, using Hess\'s calculating the value for De

Question

From the following heats of reaction, using Hess's calculating the value for Delta H for the following reaction? CS_2(l) + 3O_2(g) rightarrow CO_2(g) + 2SO_2(g) Given: C(s) + O_2(g) rightarrow CO_2(g) Delta H = -393.5 kJ/mol S(s) + O_2(g) rightarrow SO_2(g) Delta H =-296.8 kJ/mol C(s + 2S(s) rightarrow CS_2(l) Delta = 87.9 kJ/mol A toy balloon filled with air has an internal pressure of 1.25 atm at 12 degree C and a volume of 2.50 L. It 1 take the balloon to the bottom of the ocean where the pressure is 95 atmospheres. What will the new volume of the balloon be? How many moles of gas does the balloon hold?

Explanation / Answer

From the following reaction using Hess’s calculating the value for delta H for the following reaction

CS2(l) + 3O2(g) CO2 (g) + 2SO2(g)

Use Hess's Law:
H = Hf(products) - Hf(reactants)

C(s) + O2(g)--->CO2(g) H =-393.5 kJ/mol
(S(s) + O2(g)---->SO2(g)) H = -296.8 kJ/mol
C(s) +2S(s)---> CS2(l) H = 87.9 kJ/mol

C(s) + O2(g)--->CO2(g) H =-393.5 kJ/mol
2S(s) + 2O2(g)---->2SO2(g) H = -593.6 kJ/mol
CS2(l)--->C(s) +2S(s) H = -87.9 kJ/mol

Given reaction is:
CS2(l) + 3O2(g)----> CO2(g) + 2SO2(g)

H = (-393.51) + -593.6 - (89.7)

H = -1076.81 kJ

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